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Beschreibung
Mindmap von poppyekoronka, aktualisiert more than 1 year ago
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Erstellt von poppyekoronka
vor mehr als 10 Jahre
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Absorption and Emission Spectra
- Energy Levels
- An electron in a hydrogen atom can
occupy any one of the fixed energy levels
- These different energy levels are the same for all hydrogen atoms.
- In the ground state, the electrons CLOSEST to the nucleus have the lowest energy.
- The difference in the energy levels DECREASES
as the electron moves away from the nucleus
- An electron in a hydrogen atom can
occupy any one of the fixed energy levels
- Absorption Spectra
- An absorption specctra seen on earth is the VISIBLE SPECTRUM OF LIGHT,
with black lines corresponding to the absorptions of energy by the electrons
- These spectra are seen from earth when atoms
in the chromosphere around stars absorb light
- Electrons absorb a 'photon'
- Excited electrons move up to a higher energy level- they are PREMOTED.
This is what produces the lines on the Absorption spectrum
- The EM radiation absorbed by each hydrogen atom has a definite frequency, related to the difference in energy levels by AE=hv
- The EM radiation absorbed by each hydrogen atom has a definite frequency, related to the difference in energy levels by AE=hv
- Excited electrons move up to a higher energy level- they are PREMOTED.
This is what produces the lines on the Absorption spectrum
- An absorption specctra seen on earth is the VISIBLE SPECTRUM OF LIGHT,
with black lines corresponding to the absorptions of energy by the electrons
- Emission Spectra
- Black background with coloured lines on it
- These correspond to the emissions
of energy by the electrons
- These correspond to the emissions
of energy by the electrons
- An emission spectrum is seen when a chemical burns with a coloured flame
- Electrons first absorb a 'photon'
- Excited electrons move up to a higher energy level- they are premoted
- Electrons then drop back to lower energy levels. This is what produces the lines on emission spectra
- The E.R emitted by each H atom has a definite frequency related to the difference in energy levels by AE=hv
- Since AE is different for each transition, the frequency is different for each transition, and so is the colour of the lines.
- Since AE is different for each transition, the frequency is different for each transition, and so is the colour of the lines.
- The E.R emitted by each H atom has a definite frequency related to the difference in energy levels by AE=hv
- Electrons then drop back to lower energy levels. This is what produces the lines on emission spectra
- Excited electrons move up to a higher energy level- they are premoted
- Black background with coloured lines on it
- Similarities
- Both line spectra
- Lines in the same position for each element
- Lines become closer at higher frequencies
- Set of lines representing
transitions to a particular level
- Both line spectra
- Differences
- Bright lines on black background OR
black lines on coloured background
- Bright lines on black background OR
black lines on coloured background
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